This preview shows pages 1–3. Sign up to view the full content.
This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: at the origin. m can take on any value from -l to l. For our purposes, it is only important that this quantum number tells us that for each value of n there may be up to one s-orbital, three p -orbitals, five d-orbitals, and so on. For example: The s orbital ( l = 0) has one orbital, since m can only equal 0. That orbital is spherically symmetrical about the nucleus. Figure %: s orbital The p orbital ( l = 1) has three orbitals, since m = -1, 0, and 1. These three orbitals lie along the x -, y-, and z-axes. Figure %: p orbitals The d orbital ( l = 2) has five orbitals, since m = -2, -1, 0, 1, and 2. It is far more difficult to describe the orientation of d orbitals, as you can see: Figure %: d orbitals...
View Full Document
- Fall '10